The $K_{\mathrm{a}}$ for dichloroacetic acid is $3.32 \times 10^{-2} .$ Approximately what percentage of the acid is dissociated in a 0.10 M aqueous solution?
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Step 1
First, we need to write the dissociation equation for dichloroacetic acid (HCl2CO2). It dissociates in water as follows: HCl2CO2 (aq) ⇌ H+ (aq) + Cl2CO2- (aq) Show more…
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Calculate the percent dissociation for a $0.22-M$ solution of chlorous acid (HClO_, $K_{\mathrm{a}}=1.2 \times 10^{-2}$ ).
Many acids are partially dissociated into ions in aqueous solution. Trichloroacetic acid $\left(\mathrm{CCl}_{3} \mathrm{CO}_{2} \mathrm{H}\right),$ for instance, is partially dissociated in water according to the equation $$ \mathrm{CCl}_{3} \mathrm{CO}_{2} \mathrm{H}(a q) \rightleftharpoons \mathrm{H}^{+}(a q)+\mathrm{CCl}_{3} \mathrm{CO}_{2}^{-}(a q) $$ What is the percentage of molecules dissociated if the freezing point of a 1.00 $\mathrm{m}$ solution of trichloroacetic acid in water is $-2.53^{\circ} \mathrm{C}$ ?
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